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Ligand Substitution:

[Cu (H2O)6]+2
-  blue in colour
- when in reaction with H2O, displacement occurs:
[Cu (H2O)6]+2 + 2OH -> [Cu (OH)2 (H2O)4] + 2H2O
(pale blue ppt bc it's solid, neutral charge)
- when [Cu (OH)2 (H2O)4] reacts with concentrated ammonia:
[Cu (OH)2 (H2O)4] + 4 NH3 -> 2OH- + 2H2O + [Cu (NH3)4 (H2O)2]
(+2 bc charge summary, ppt of deep blue colour)

- when [Cu (H2O)6]+2 reacts with Cl-
[Cu (H2O)6]+2 + Cl- -> 6H2O +   [Cu(Cl)4 ]-2
(yellow in colour)

[Co(H2O)6]+2
- pink in colour

- when reacting with OH-
[Cu (H2O)6]+2 + 2OH- -> [Cu (OH)2 (H2O)4] + 2H2O
(blue/green)
if [Cu (OH)2 (H2O)4] is heated, becomes red bc all the H2O evaporates to make (Co(OH)2)

- when reacting with NH3
[Cu (H2O)6]+2  + 6NH3 -> 6H2O + [Cu (NH3)6]+2
(straw-coloured)

- When reacting with Cl-
[Cu (H2O)6]+2 + 4Cl -> 6H2O + [Cu (Cl)4]-2
(blue solution)

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Transition elements : d block elements that forms one/more stable ions with an incomplete d subshell

Sc & Zn are not transition metals. Why ?

Sc only forms Sc3+

Does not have an incomplete d subshell in the ions (ends at 3d0)

Zn only forms Zn2+

Does not have an incomplete d subshell in the ions (ends at 3d10)

Write the electronic configuration for Cu

1. Cu : [Ar] 4s1  3d10

2. Cu+ : [Ar] 4s0  3d10 → not a transition metal

3. Cu2+ : [Ar] 4s0  3d9 → has an incomplete d subshell, a transition element

Properties of transition metals

Variable oxidation states

Cu : Cu+, Cu2+, etc

Catalyst : transition metals as homogeneous catalyst (involving changes in oxidation numbers)

Form complex ions

Form coloured compounds

Different oxidation number, different colour

Fe2+ (green), Fe3+ (brick-red)

Physical properties of transition metals

High melting points

High densities

Hard and rigid, useful in construction materials

Good conductors of electricity and hear

Ionisation energy, atomic radius and ionic radius across the period remains almost constant (no variety)

Ligands and complex formation

Ligand is a species that contains a lone pair of electrons that forms a dative bond to central metal atom/ion

Complex is a molecule or ion formed by a central atom/ion surrounded by one or more ligands

Type of ligands

1. Monodentate [one coordinate bond]

1. Water

2. Ammonia

3. Cl-

4. CN-

2. Bidentate [two coordinate bonds]

1. 1,2-diaminoethane

2. Ethanedioate ion

3. Polydentate [three coordinate bonds]

1. EDTA4-

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Transition elements - metals found in d block that has incomplete d orbitals
Scandium not transition element because :
- only forms Sc3+
- Sc3+ has no electrons in 3d subshells
Zinc not transition element because :
- only forms Zn2+
- Zn2+ has complete 3d subshell

Properties of transition element :
- variable oxidation state
- behave as catalysts
- form complex ions
- form colored compounds

Ligands -> molecules or ions surrounding the central metal atom/ion

Monodentate ligands :  forms 1 coordinate bond with central metal ion
Bidentate ligands : forms 2 coordinate bonds with central metal ion
Polydentate ligands : forms 2 or more coordinate bonds with central metal ion

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Learnt:
Zinc and scandium are not transition elements due to having incomplete d subshells
-Properties of transition elements:
1. Have variable oxidation states
2. Form color compounds
3. High density
4. Act as a catalyst
5. Form complex ions
6. Hard and Rigid
7. High melting point

The shape of 3dxy and 3dz2
-Ligands are a species that contains a lone pair of electrons that form coordinate bonds

- Complex ion are molecule or ion where the central atom is surrounded by one or more ligands.

- 2 types of ligands:
1. Monodentate (One ligand can form 1 coordinate bonds)
2. Polydentate (One ligands can form more than 1 coordinate bonds)

# data[].attributes.body
Transition Metals

a d block element that forms one or more stable ions with an incomplete d subshell

Sc and Zn are not transition metals

Properties of Transition Metals

Variable Oxidation state

Behaves as catalyst

Form complex ions

Form coloured compounds

High melting point

High density

Hard and rigid

Good conductors of electricity and heat

1st ionisation energy, atomic radius and ionic radius do not vary across first row

Ligands and complex formations

Ligand is a species that contains a loner pair of electrons that forma a dative bond to a central metal ion

Complex is a molecule or ion formed by a central atom/ion surrounded by one or more ligands

Co-ordination number is the number of co-ordinate bonds to the central metal ion

Types of ligands : Monodentate(1 co-ordinate bond), Bidentate(2 co-ordinate bond), Polydentate(2 or more co-ordinate bond)

We also learnt more about geometry of transition complex and the colour of complexes.

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Learnt:
-zinc and scandium are not transition elements due to having incomplete d subshells
-Properties of transition elements:
1. Have variable oxidation states
2. Form color compounds
3. High density
4. Act as a catalyst
5. Form complex ions
6. Hard and Rigid
7. High melting point
-the shape of 3dxy and 3dz2
-Ligands are a species that contains a lone pair of electrons that form coordinate bonds
- Complex ion are molecule or ion where the central atom is surrounded by one or more ligands.
- 3 types of ligands:
1. Monodentate (One ligand can form 1 coordinate bonds)
2. Polydentate (One ligands can form more than 1 coordinate bonds)

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A transition element is a d-block element that forms one or more stable ions with an incomplete d subshell. Scandium and Zinc are not transition element because there will be no electron left or the number of electron will be complete in the d subshell. D subshell have 5 different orbital, each of them can contain 2 electron. Most of the transition metals have multiple oxidation states. Transition elements act as a catalyst and they form coloured compounds. Transition elements have high melting/boiling points and are also hard and rigid. Transition metal’s 1st ionization energy do not vary across the first row. In octahedral complexes, there are six ligands arranged around the central metal ion and in tetrahedral complexes, there are four ligands arranged around the central metal ion. The non-degenerate orbitals in tetrahedral complexes are at a lower and stable energy  and there is also less repulsion between the 3dx2-y2 and 3dz2 orbitals. The non-degenerate orbitals in octahedral complexes are at a higher energy and there is more repulsion between 3dx2-y2 and 3dz2.

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Transition elements are d-block elements that form one or more stable ions with an incomplete d subshell. Scandium and Zinc are not transition metals as they do not have incomplete d subshells. I also learned about the properties of transition metal, what ligands are, what complex molecules and ions are, what a coordination number is, and how tetrahedral and octahedral split.

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Transition elements are d-block elements which form one or more stable ions with an incomplete d subshell.

Scandium and Zinc are not transition elements as their cations do not have incomplete d subshells.

Transition elements have these properties:

1. Have variable oxidation states

2. Behave as catalysts

3. Form complex ions

4. Form colored compounds

5. High melting points

6. High densities

7. Hard & Rigid

We also need to learn how to draw the shape of 3dxy and 3dz2 orbitals.

Ligands are a species that contains a lone pair of electrons that forms a coordinate dative bond to a central metal ion.

A molecule/ion formed by a central atom/ion surrounded by one or more ligands is a complex ion/compound.

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Transition elements are d-block elements that form one or more stable ions with an incomplete d subshell.

Scandium and Zinc arre not transition metals as zinc has a complete subshell while scandium has an empty subshell

Transition metal properties
-Variable oxidation states
-acts as catalysts
-can form coloured complex compounds
-good conductor of heat and electricity
-high density and melting point
-hard and rigid
-1st IE, atomic and ionic radius do not vary across first row

ligands- a species that contains a lone pair of electrons that forms co-ordinate dative bonds with the central metal atom/ion

complex-molecule/ion formed by a central atom/ion surrounded by one or more ligands

co-ordination number-number of co-ordinate dative bonds to the central metal ion

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Zinc and Scandium are not transition elements because they only have one stable ion

Shapes of d orbitals

Transition metals have variable oxidation state, behave as catalyst, form coloured compounds (absorbs part of the visible spectrum), high mp and bp, conducts electricity

Ligands (species that contains a lone pair of electron that forms a dative bond to the central metal ion)
-Monodentate (single bond)
-Bidentate (double bond)
-Polydentate (more than two bonds)

Dont really understand splitting

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We learnt about transition elements and their definition: d-block elements that can form 1 or more ions with an incomplete d subshell

We learnt how to graph different shapes of d orbitals,
(ex: dxy,dyz,dxz,dx^2-y2,.)

The properties of transition metals

High MP

Good conductor of electricity

Makes coloured compounds

Act as catalysts

High density

Hard and rigid

Form complex ions

Ligand is a species that contains a lone pair of electrons that forms a dative bond to a central metal atom/ion.

Complex is a molecule or ion formed by a central atom/ion surrounded by one or more ligands.

The reason is that the energy levels for d orbitals and the proceeding s orbitals are very similar, so both orbitals can be used for bond formation.

The types of ligands are monodentate, bidentate and polydentate

Coordination number is the number of coordinate bonds to the central metal ion.

Complexes can split into degenerate and non-degenerate orbitals

In octahedral complexes, 3dxy and 3dz2 will experience greater repulsion and will be splitting into non-degenerate orbitals at higher energy level while in tetrahedral complexes, 3dxy and 3dz2 will experience less repulsion and will be splitting into non-degenerate orbitals at lower energy level

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Today we discussed about transtition metals

Properties

High MP

Good conductor of electricity

Makes coloured compounds

Act as catalysts

High density

Hard and rigid

Form complex ions

Ligands and Complex formations
- Ligands are a species that has a lone pair of electrons and forms a dative bond with a central ion

- complex molecules are molecules with a central ion surrounded by ligands

- The number of co-ordinate bonds to a central ion is the co-ordinate number

Ligands
- Monodentate (1 co-ordinate bond)
- Bidentate (2 co-ordinate bond)
- Polydentate (2 or more co-ordinate bond)

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What we learned:
- Definition of transition elements
-Sn and Zn are not transition elements because they only form one stable ion. They are also colorless because
-How to draw shapes of 3dxy orbital and 3dz orbital.
-Properties of transition metals
-Transition metals act as catalysts because they have variable ON.
-Ligand is a species that contains a lone pair of electron that form a dative bond to a central metal ion.
- Complex is a molecule or ion formed by a central ion surrounded by one or more ligands
- Co-ordination number is the number of co-ordinate bonds to the central metal ion
- Types of ligands : Monodentate, bidentate (one ligand can form 2 co-ordinate bonds), polydentate (one ligand can form more than 2 co-ordinate bonds)
- Octahedral complex has more repulsion and 3d x2-y2 and 3d z2 has slightly higher energy level than the other orbitals.
-How do transition elements get their colour? Different ligands causes the d orbitals to split by a different amount of energy. The energy corresponds to the energy part of the visible spectrum of light. The electrons in either non-degenrate orbitals absorb the energy and complementary color is seen.

# data[].attributes.body
Today we discussed about transition metals and their properties.

Transition metals are elements that is located in the d-block of the periodic table.

They are 7 properties that include: High melting point, hard and tough, ability to form colored compounds, high density, variable oxidation state, as well as good conductor of heat and electricity.

We also learnt about ligands. There are three types of ligand: Monodentate, Bidentate and Polydentate. Mono means 1 coordinative bond, Bi means 2 and so on.

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Transition Metals

a d block element that forms one or more stable ions with an incomplete d subshell

Sc and Zn are not transition metals

Properties of Transition Metals

Variable Oxidation state

Behaves as catalyst

Form complex ions

Form coloured compounds

High melting point

High density

Hard and rigid

Good conductors of electricity and heat

1st ionisation energy, atomic radius and ionic radius do not vary across first row

Ligands and complex formations

Ligand is a species that contains a loner pair of electrons that forma a dative bond to a central metal ion

Complex is a molecule or ion formed by a central atom/ion surrounded by one or more ligands

Co-ordination number is the number of co-ordinate bonds to the central metal ion

Types of ligands : Monodentate(1 co-ordinate bond), Bidentate(2 co-ordinate bond), Polydentate(2 or more co-ordinate bond)

We also learnt more about geometry of transition complex and the colour of complexes.

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nucleus controlling electron closer to itself so we expect to increase. increase not significant (radius and ie appear almost the same)

fe ligands octahedral

cyanide nickel ligands square planar

cobalt tetrahedral

ligands - species containing an electron lone pair forming a dative bond to a central metal atom/ion

complex - molecule/ion formed by central atom

coord number - no of cord bonds bond to cnetral atom

monodentate - coordinate bon only one (h2o, ammo, cl-, cn-)

bi - two coord (1,2-diaminoethane en, ethanedioate ion)

poly - more than two (edta4-)

colour // 5d degenerate (same energy level) // coord split into two sets - non degenerate orbitals

SPLIT INTO TWO

OCTAHEDRAL (DEGENERATE) light absorb energy

tetrahedral

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A transition metal

- a d block element that forms one or more stable ions with an incomplete d subshell

- between group 2 and 13

- outermost electron end at that orbital

- Sc and Zn are not considered

Properties of Transition Metals

1. Variable oxidation states

( examples Fe2+ and Fe3+)

(note: not all of them such as nickel but they are still transition metals as long as they satisfy the defenition)

-> the reason is because of the similarity in energy of the 3d and the 4s subshells

2. Behave as catalysts

-> homogenous catalysts

3. Complex ions

4. Form coloured compounds

-> because of complex ions

5. High melting points

6. High density

7. Hard and rigid

8. Good conductors of electricity and heat

-> metal

9. 1st IE, atomic and ionic radius do not vary across first row

-> across period, atomic radius is getting smaller and smaller because proton numbers while shells remain constant so nucleus will attract the electrons and become closer so radius is smaller

-> IE is supposed to increase but the increase is not significant

Lipids and Complex Formations

• contains a lone pair of electrons

• lone pair forms a dative bond to a central metal ion

• complex is a molecule or ion form by a central atom surrounded by more ligands

• co-ordination number is the number of co-ordinate binds to the central metal ion

> Fe2+ has a co-ordination number of 6

> Ni2- has a co-ordination number of 4

> Co2- has a co-ordination number of 4

> based on total number if co-ordinate bond that is being formed to the central ion

Colour of Complexes
• part of visible spectrum is absorbed by transition metal complex
• 5d orbitals in transition metals or ions as degeneratewhich means same energy levels
• all 5 orbitals have same energy level
• co-ordinate bonding with ligands will cause the orbitals to split into two sets
> because of the split they are going to form non degenerate orbitals which means different level of energy
• from having one energy level, they will then have two different energy levels so they will have different colour

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Major subtopics reviewed in the video:

- the standard definition of transition metals
- Sc and Zn as outliers
- physical properties of transition metals
- chemical properties of transition metals
- the standard definition of ligands
- ligands in the formation of complex ions with transition metals
- types of ligands ( depending on the number of coordinate bonds a ligand has with a central transition metal)
- tetrahedral and octahedral complex ions
- splitting of degenerate d orbitals into non degenerate orbitals
- the formation of coloured complexes due to the absorption of specific wavelengths of light by electrons as they move into higher energy levels

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I learned about:
- properties of transition elements
- why Sc and Zn are not transition elements
- D block and its electronic configuration
- how to draw d orbital
- Ligands and complex ions
- types of ligands
- splitting

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transition element

a d-block element that is capable of forming one or more stable ions with an incomplete d subshell

scandium forms only Sc³⁺, hence its electronic configuration becomes [Ar] 3d⁰ 4s⁰, thus it has an unoccupied d subshell, which explains why it is not a transition element

zinc forms only Zn²⁺, hence its electronic configuration becomes [Ar] 3d¹⁰ 4s⁰, thus it has a complete d subshell, which explains why it is not a transition element

shapes of orbitals

dxy

dyz

dxz

dx²-y²

dy²-z²

dx²-z²

dz² is a combination of dy²-z² and dx²-z²

properties of transition metals

1. variable oxidation states

similar energy levels for 4s and 3d subshells, hence electrons can be removed from them

2. behave as catalysts

3. form complex ions

4. form coloured compounds

5. high melting points

6. high densities

7. hard and rigid

8. good conductors of electricity and heat

9. 1st ionisation energy, atomic radius, and ionic radius do not vary across the first row

ligand

a species that contains a lone pair of electrons that forms co-ordinate dative bonds with the central metal atom/ion

complex

molecule/ion formed by a central atom/ion surrounded by one or more ligands

co-ordination number

number of co-ordinate dative bonds to the central metal ion

types of ligands

1. monodentate

one co-ordinate dative bond

2. bidentate

two co-ordinate dative bonds

3. polydentate

more than two co-ordinate dative bonds

geometry of transition complexes

1. co-ordination number 2

linear

180⁰

2. co-ordination number 4

square planar

90⁰

3. co-ordination number 4

tetrahedral

109.5⁰

4. co-ordination number 6

octahedral

90⁰

colour of complexes

all 5 d orbitals in transition metals are degenerate (same energy levels)

co-ordinate dative bonding with ligands cause the orbitals to split into two sets of non-degenerate orbitals

energy is absorbed from the visible light spectrum and this causes the electron to be excited which gives a complementary colour

octahedral complexes

3dxy and 3dz² experience greater repulsion than other orbitals, hence they will split and move to a higher energy level

tetrahedral complexes

3dxy and 3dz² experience less repulsion than other orbitals, hence they will split and move to lower energy level

different ligands cause the d orbitals to split by different amounts of energy

different colours are absorbed from the visible light spectrum and complementary colours are seen

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Transition elements are d-block elements that form one or more stable ions with an incomplete d subshell

Sc and Zn are not transition elements as they don't have an incomplete d subshell, Sc has no electrons in the d subshell while Zn has 10 electrons (complete) d subshell

Properties of transition metals

Variable oxidation states

Behave as catalysts

Form complex ions

Form coloured compounds

High melting points

High densities

Hard and rigid

Good conductors of electricity and heat

1st IE, atomic and ionic radius do not vary across the first row

Ligands and complex ions

Ligand is a species that contains a lone pair of electrons that forms a dative bond to a central metal atom/ion

Complex is a molecule/ion formed by a central atom/ion surrounded by one or more ligands

Co-ordination number is the number of co-ordinate bonds to the central metal ion

Fe2+ forms six dative/co-ordinate bonds

Water molecules that will give lone pairs of electrons are called ligands

The resulting ion is called complex ion

Ni2+ forms four dative/co-ordinate bonds with CN- ions

CN- ions are called ligands

Types of ligands

Monodentate: one co-ordinate bond, example: water, ammonia, Cl-, CN-

Bidentate: two co-ordinate bonds, example: 1,2-diaminoethane - NH2CH2CH2NH2 (en), Ethanedioate ion, C2O42-

Polydentate: more than two co-ordinate bonds, example: EDTA4-

Colour of complexes

Part of the visible spectrum is absorbed by the transition metal complex

5d orbitals in transition metals or ions are described as degenerate, same energy level

The coordinate bonding with the ligands causes the orbitals to split into two sets of non-degenerate orbitals

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During the lecture, i have learnt about transition elements.

I learnt about

the definition of transition element(d-block)

Why Scandium and Zinc are not transtion metals

Shape of specific orbitals

Properties of transition metals

Ligands and complex ions

Types of ligands

Colour of complexes

How to count coordination number

Octhahedral/ tetrahedral complexes

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- Transition elements are d-block elements, whose cations have incomplete d subshells.
- this means that Sc and Zn cations are not transition metals (their common cations generally do not have incomplete d subshells)
- properties of transition metals:
- multiple oxidation states (meaning that they can be homogenous catalysts!)
- colored compounds, colors obtained from absorbing part of the visible spectrum by only transition complexes
- are catalysts
- ionization energy, ionic and atomic radius does not vary much across the period
- high density, melting and boiling points, hard and rigid, good electrical and heat conductors (not ad important but oh well)

- very cool looking d orbits shapes, can't draw them but there is a donut, electron clouds aligned to the axes, and across the axes.
- complex bc ligands can bond to transition metals!
- ligands can form coordinate dative bonds with the metals, which is possible bc of empty d sub shells
- overall charge is both the ligands charge and the transition metals' charge (h20 is neutral)
- types of ligands (monodentate = 1, didente = 2, polydente= many)
- shapes formed by complex compounds! Square planar, octahedral (bc 8 sides, 6 bonds), linear, basically molecular shapes

- splitting: produces two degenerate orbitals, electrons cannot be promoted to higher levels, no different absorptions. Degenerate orbitals can also be produced, electrons do not move anywhere, therefore no different absorptions.

I need to memorize the shapes as well as the bond angles. If you asked me anything about degenerative orbitals i honestly cannot answer bc i know nothing? What even is degenerative/generative, and how does that make different absorptions? I understand the parts where the electrons cannot move bc of the full subshells tho

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from the lecture, I learned:

transition element :
- d-block element that forms one or more stable ion with an incomplete d subshell
- scandium and zinc are not transition metals
- multiple oxidation states (similar energy level of 3d and 4s)
- behave as catalysts
- form complex ions
- form coloured compounds
- high mp and density
- hard and rigid
- good conductors of electricity and heat

ligands and complex formations
- ligands are species that has lone pair of electrons to form dative bonds to a central atom / ion
- complex is a molecule / ion formed by central atom / ion
- co-ordinate number is the number of co-ordinate bonds
- Fe2+ form 6 dative bonds (octahedral shape ~ water molecules as ligands)
- Ni2+ form 4 dative bonds (square planar shape ~ CN- as ligands)
- Co2+ form 4 dative bonds (tetrahedral shape ~ Cl- ions as ligands)

types of ligands
- monodentate ( one co-ordinate bond )
- bidentate ( two co-ordinate bonds )
- polydentate (more than 2 co-ordinate bonds )

colour of complexes
- degenerate = same energy
- non-degenerate = different energy
- coordinate bonding between ligands causes orbitals to split into two sets of non-degenerate orbitals
- in octahedral, 3dxy and 3dz2 have more repulsion , so it splits to higher energy levels
- in tetrahedral, 3dxy and 3dz2 have less repulsion , so it splits to lower energy levels

I need to learn more in the colour of complexes and practice more questions regarding this topic. However, the lecture was clear as always and cleared my doubts.

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Transition Metals
- d-block element
- Forms one or more stable ions with an incomplete d subshell
- Does not include Sc & Zn

Orbitals
- Always follow alphabetical order (x, y, z)

Properties
- Variable oxidation states
- Catalyst
- Form complex ions
- Form colored compounds
- High mp
- High density
- Good electrical conductor
- Good heat conductor
- Hard
- Rigid

Ligands
- Contains 1 lone pair
- Forms a dative bind to a central metal atom

Coordination Number
- Number of coordinate bonds formed by central atom

Monodentate Ligand
- 1 coordinate bond
- Ex : H2O, NH3

Bidentate Ligand
- 2 coordinate bond

Polydentate Ligand
- More than 2 coordinate bonds

# data[].attributes.body
Transition metals : d-block element that forms one or more stable ions with an incomplete subshell
- Have variable oxidation states
- Behave as catalysts
- Form complex ions & coloured compound
- Property of metal
- !! Zn & Sc are not !!
* Sc : Only form Sc3+ (no electron -> can't absorb light) , d subshell is empty
* Zn : Only form Zn2+ (orbitals are complete -> electrons can't go into "excited" state)
- High melting point & density
- Rigid and Hard
- Good conductor of electricity and heat

Ligands
1. Monodentate : dative by a single lingand
2. Bidentate : 2 dative
3. Polydentate : more than 2 dative

Need to read textbook for introduction, a bit of information overload. Get familiar with the terms.

# data[].attributes.body
what i learnt:

d block elements that forms one or more stable ions with an incomplete d subshell.

scandium and zinc are not included in transition metals

transition metals has a good conductor of electricity and heat

transition metals have high melting point and density

they are hard(rigid), And good for construction materials

there are only a small variation of atomic,ionic radius and ionization energy

transition metals behave as catalysts

they can form complex ions

And they can form coloured compounds

we always remove the electrons from the S orbitle then the D orbitle.

special cases:

Cu= 4s1 3d10       Cr= 4s1 3d3

Cu+= 4s0 3d10    Cr3+ = 4s0 3d3

Cu2+= 4s0 3d9    Cr6+= 4s0 3d0

Ligands

A species that contains a lone pair of electrons that forms a dative bond to a central metal ion

types of ligands: monodentate, bidentate and polydentate

Complex

A molecule formed by a central ion surrounded by one or more ligands

Co ordination number

the number of coordinate bonds to the central metal ion

different shapes of D orbitals:

Xy

Xz

Yz

X2Y2

Z2

I think i need to revise more on the splitting of complexes, ligand structure and memorizing their shapes.

Overall the lesson was clear and detailed as usual

# data[].attributes.body
-  Transition metals are defined as a d block element tat forms one or more stable ions with an incomplete d subshell
- Sc and Zn are not Transition metals
- Transisiton metals have variable oxidation states, behave as catalysts, form complex ions, form coloured compounds and also has a property of a usual metal.
-  shapes of d orbital, 3dxy, 3dz^2
- Ligands, Co-ordination number,  complex, types of ligands, 3 types of ligands, splitting of complexes.

# data[].attributes.body
-Transition elements are d-block elements that can form 1 or more ions with an incomplete d subshell

-Shapes of d orbitals,(dxy,dyz,dxz,dx^2-y2,.)

- properties of transition metals

-Ligands and complex ions

-types of ligands: monodentate, bidentate and polydentate

-Splitting of complexes, splits into degenerate and non-degenerate orbitals

-In octahedral complexes, 3dxy and 3dz2 will experience greater repulsion and will be splitting into non-degenerate orbitals at higher energy level

-In tetrahedral complexes, 3dxy and 3dz2 will experience less repulsion and will be splitting into non-degenerate orbitals at lower energy level

# data[].attributes.body
Transition Metals

A d-block element that forms one or more stable ions with an incomplete d subshell.

When forming ions, remove from 4s subshell first.

Sc is not a transition metal  as Sc only forms Sc3+ with electronic configuration [Ar] 4s0 3d0, where the d subshell is empty.

Zn is not a transition metal as Zn only forms Zn2+ with electronic configuration [Ar] 4s0 3d10, where the d subshell is full.

Orbital Shape

s: spherical

p: dumbbell

d: clover

“balloon” in the middle: dxy, dxz, dyz

“balloon” in the axis: x2-y2, x2-z2, y2-z2

“balloon” in the x and y axes form a clover, which moves around to form a donut shape, dz2

Properties of Transition Metals

1. Variable oxidation states (at least 1 stable ion with incomplete d subshell), since 4s and 3d have similar energy levels

Mn: [Ar] 4s2 3d5, its maximum oxidation state is 7+ since the next electron would need to be removed from the 3p subshell, which is closer to the nucleus.

4s and 3d, 5s and 4d, 6s and 5d have similar energylevels

1. Behave as catalysts

2. Form complex ions

3. Form coloured compounds

4. High melting point

5. High density

6. Hard and rigid

7. Good conductor of electricity and heat

8. 1st IE, atomic radius, and ionic radius do not vary too much across the period

Ligands and Complex Formations

Fe2+ forms 6 dative bonds

Each water molecule donates an electron pair to the Fe atom

Octahedral shape (8 faces)

Ni2+ forms 4 dative bonds with CN-

CN- are ligands

Square planar

Co2+ forms 4 dative bonds with Cl-

Cl- are ligands

Tetrahedral (depends on size)

Ligands contain a lone pair of electrons that form a dative bond to a central metal atom

Coordination number: number of coordinate bonds formed by the central atom

Types of ligands: monodentate (1 dative by a single ligand), bidentate (2 dative), polydentate (more than 2)

The coordinate bonding with ligands causes the orbitals to split into two sets of non-degenerate orbitals.

Octahedral: Degenerate orbitals separate into two non-degenerate orbitals. The electrons absorb light energy and move to the excited state, absorbing light energy, giving a complementary colour. 3dxy and 3dz2 will experience greater repulsion, pushing the electrons to a higher energy level.

Tetrahedral: Split into non-degenerate but the repulsion is not as great so it is lifted to an energy level lower than that of octahedral compounds.

Colour Complexes

Different ligands split the d orbitals by different amounts of energy.

Different colours are absorbed by visible light so their complementary colours are seen.

Zn2+ and Sc3+ are colourless

Sc3+: No electrons in 3d to absorb light.

Zn2+: The orbitals are complete so the electrons cannot go to their excited state.

I think I need to revise more on the ligand structure and memorise their shapes, and read more about the colour complexes. Teaching was quite fast for me but still elaborate.

# data[].attributes.body
From today's lecture, I learnt about:
Transition Elements

d block element that forms one or more stable ions with an incomplete d subshell

scandium and zinc are not transition metals, this is because scandium forms Sc3+ where its' d subshell is empty while zinc forms Zn2+ where its' d subshell is full

drawing the shapes of d orbitals, specifically 3dxy and 3dz2 orbitals

Properties of Transition Metals

1. variable oxidation states

2. behave as catalysts

3. form complex ions

4. they form coloured compounds

5. high melting points and densities

6. hard and rigid

7. good conductors of electricity and heat

8. small variation in 1st IE, atomic radius & ionic radius

Ligands and Complex Formations

Ligand is a species that contains a lone pair of electrons that forms a dative bond to a central metal atom/ion

Complex is a molecule or ion formed by a central atom/ion surrounded by one or more ligands

Co-ordination number is the number of co-ordinate bonds to the central metal ion

The formations of complexes of copper(II) and cobalt(II) ions with water and ammonia molecules and hydroxide and chloride ions

Types of Ligands

monodentate (one co-ordinate bond) (H2O, NH3, Cl- and CN-)

bidentate (two co-ordinate bonds) (1,2-diaminoethane-NH2CH2CH2NH2(en), Ethanedioateion, C2O42-)

polydentate (more than two co-ordinate bonds) (EDTA4-)

Geometry of Transition Complex

Splitting of Complexes

The coordinate bonding with ligands causes the orbitals to split into two sets of non-degenerate orbitals

In octahedral complexes, 3dxy and 3dz2 will experience greater repulsion and will be splitting into non-degenerate orbitals at higher energy level

In tetrahedral complexes, 3dxy and 3dz2 will experience less repulsion and will be splitting into non-degenerate orbitals at lower energy level

I think I need to revise more on the splitting of complexes and past year paper questions to fully understand this chapter. But overall, everything was clear and it was easy to follow and understand the lecture.

# data[].attributes.body
Learnt about :
- properties of transition metals
- why scandium and zinc are not considered transition metals
- drawing of the d orbitals
- what are ligands, co-ordination number, and complex
- the three types of ligands
- splitting of the complexes

Need to revise more on :
Splitting of complexes

Teaching was fast but quite clear